Home Journals Articles Updates About
CN
image
收藏切换
Selective adsorption behaviors of CO2 in small-pore chabazite zeolites
收藏切换
PDF
Fubin PENG1, Shenyong REN1, *, Jiujiang WANG2, Shangshu LIU1, Xin TAO1, Hongjuan ZHAO2, Honghai LIU2, Min GU1, Xiaodan ZHU1, Can CUI1, Baojian SHEN1, Chunming XU1
Journal of Fuel Chemistry and Technology | 2026, 54(9) : 20250397-1849 - 20250397-1860
Less
收藏切换
Journal of Fuel Chemistry and Technology | 2026, 54(9): 20250397-1849-20250397-1860
• RESEARCH PAPER •
Selective adsorption behaviors of CO2 in small-pore chabazite zeolites
Full
Fubin PENG1, Shenyong REN1, *, Jiujiang WANG2, Shangshu LIU1, Xin TAO1, Hongjuan ZHAO2, Honghai LIU2, Min GU1, Xiaodan ZHU1, Can CUI1, Baojian SHEN1, Chunming XU1
Affiliations
  • 1State Key Laboratory of Heavy Oil Processing, CNPC Key Laboratory of Catalysis, School of Chemical Engineering and Environmental Science, China University of Petroleum (Beijing), Beijing 102249, China
  • 2CNPC Key Laboratory of Catalysis, Petrochemical Research Institute, Lanzhou 730060, China
About Author:

#

：These authors contributed equally to this work.

Published: 2026-09-10 doi: 10.1016/S1872-5813(26)60687-1
Outline
收藏切换

Chabazite-type (CHA) zeolite is considered to be a highly promising CO2 adsorption material due to is unique pore structure. However, the underlying adsorption kinetics of CHA zeolite still need to be studied to facilitate development of efficient adsorbents. In this study, the preparation method, CO2 adsorption kinetics, and thermodynamic properties of CHA zeolite are investigated. CHA zeolite is synthesized from hydrogen type faujasite-type (H-FAU) zeolite using a transformation method. By modulating the ratios of n(KOH)/n(SiO2), n(H2O)/n(SiO2), crystallization temperature, and crystallization time during the synthesis process, the optimal synthesis conditions for CHA zeolite are explored based on X-Ray Diffraction (XRD) and scanning electron microscopy (SEM) of the as-synthesized materials. The CO2 adsorption performance of the prepared CHA zeolite is tested and evaluated using both dynamic and static measurements. Different kinetic models are applied to analyze the kinetic behavior of the adsorption process. Among them, the Avrami equation yields a good fit to illustrate the adsorption process of studied zeolites (R2 > 0.99). With increasing temperature, the adsorption process reach equilibrium more quickly due to the enhanced adsorption rate. The selectivity also increases with increasing temperature, indicating that the adsorption process of CO2 on CHA zeolite is mainly controlled by diffusion. Breakthrough data and thermodynamic analysis show that the material’s interaction with CO2 is stronger than that with N2, yet the CO2 adsorption is still dominated by physical interactions. The weak adsorption strength between CO2 and CHA zeolite is conducive to gas desorption. These findings provide a theoretical support for optimizing industrial adsorption operating conditions.

chabazite  /  CO2 adsorption  /  zeolite crystallization  /  adsorption kinetics  /  Avrami model
彭福斌, 任申勇, 王久江, 刘尚书, 陶欣, 赵红娟, 刘宏海, 谷敏, 朱晓丹, 崔粲, 申宝剑, 徐春明. 小孔菱沸石选择性吸附CO2的性能研究. 燃料化学学报（中英文）, 2026 , 54 (9) : 20250397-1849 -20250397-1860 . DOI: 10.1016/S1872-5813(26)60687-1
Fubin PENG, Shenyong REN, Jiujiang WANG, Shangshu LIU, Xin TAO, Hongjuan ZHAO, Honghai LIU, Min GU, Xiaodan ZHU, Can CUI, Baojian SHEN, Chunming XU. Selective adsorption behaviors of CO2 in small-pore chabazite zeolites[J]. Journal of Fuel Chemistry and Technology, 2026 , 54 (9) : 20250397-1849 -20250397-1860 . DOI: 10.1016/S1872-5813(26)60687-1
Full Text
Less
Accelerated industrialization has driven a sustained increase in atmospheric CO2 concentrations, which constitutes one of the dominant contributing factors to global climate warming and frequent occurrences of extreme weather event[1]. In response to this pressing global challenge, both the international and the scientific efforts are overwhelmingly directed towards CO2 capture and emission reduction technologies. Among various approaches, adsorptive capture stands out as a promising strategy for CO2 removal, which has garnered extensive research attention owing to its operational simplicity and relatively low energy consumption[2−3].
Zeolitic molecular sieves are widely regarded as ideal adsorbents for CO2 capture with attributes of unique microporous architecture, high specific surface area, excellent thermal and chemical stability, and tunable pore size dimensions. As such, these inorganic porous silicate materials demonstrate great potential in efficient CO2 capture via physical adsorption mechanisms[3−5].
As a representative eight-membered ring small-pore zeolite, CHA-type framework exhibits remarkable potential in gas adsorption and separation applications due to its distinctive topology and precisely engineered pore architecture. Particularly notable are its exceptional performance characteristics demonstrated in greenhouse gas capture and noble gas purification processes[6]. Specifically, CHA zeolite exhibit exceptional adsorptive capacity toward critical atmospheric species including carbon dioxide (CO2)[7], methane (CH4)[8] and nitrous oxide (N2O)[9]. This excellent adsorption capacity and separation selectivity are largely attributed to the unique “trapdoor effect” or “molecular sieve effect” of CHA zeolite[10]. The “trapdoor effect” refers to the ability of the pores or cage-like windows of CHA zeolite molecular sieves to undergo reversible structural dynamic changes under specific conditions based on the size and shape of the adsorbate molecules, thereby achieving selective adsorption and blocking of specific molecules[11]. This effect allows CHA zeolite to precisely distinguish gas molecules of different sizes and polarities. For example, in CO2 capture, CHA zeolite can effectively and selectively adsorb CO2 from a mixed gas stream, while its adsorption capacity for other gases (such as N2) is relatively low. This characteristic is of great significance for achieving efficient and low-energy greenhouse gas emission reduction. In addition to greenhouse gases, CHA zeolite molecular sieves have also shown significant potential in the field of rare gas separation. For example, in the separation of xenon (Xe) and krypton (Kr), traditional methods such as cryogenic distillation are energy-intensive and complex to operate due to the subtle differences in the molecular size and polarity of the two gases. CHA zeolite molecular sieves can effectively distinguish between these two rare gases by leveraging their pore structure, achieving an efficient Xe/Kr separation. This characteristic of CHA zeolites provides a new approach for nuclear industry waste gas treatment, isotope separation, and the production of high-purity rare gases[12].
Carbon dioxide, as the leading greenhouse gas, contributes significantly to the greenhouse effect. In their research of carbon dioxide adsorption on CHA zeolite, Clatworthy et al.[7] synthesized micron- and nano-scale K-CHA zeolites using a hydrothermal method. By comparing the steepness of the breakthrough curves and performing derivative analysis, a comparative study of the adsorption kinetics was conducted to evaluate the relative adsorption rates of nanoscale and microscale CHA zeolites. Studies have found that reducing the size of zeolite crystals can significantly shorten the diffusion path of CO2 molecules and reduce the diffusion resistance of micropores, thereby enhancing the overall mass transfer performance and effectively improving the efficiency of the rapid separation process. Fu et al.[13] achieved high adsorption performance by controlling the distribution of Zn2+ in the six-membered rings (6MRs) of zeolite: when Zn2+ is located at the paired anion sites of 6MRs, the adsorption capacity reaches 0.51 mmol/g (Si/Al≈7), which is 17 times higher than that of H-type zeolite; after reducing the Si/Al ratio to ~2, the capacity increases to 0.67 mmol/g. By comparing the steepness of breakthrough curves with those of 13X zeolite, the modified Zn-CHA zeolite exhibited relatively faster adsorption kinetics. Cao et al.[14] synthesized a sunflower-shaped CHA zeolite superstructure (SFS-CHA) through a directional attachment mechanism, which is based on self-assembly of nanocrystals to form a micro-mesoporous hierarchical structure. The material exhibits a CO2 adsorption capacity of 71.14 cm3/g at 298 K and 0.15 bar, and IAST predicts CO2/N2 and CO2/CH4 selectivity of 815 and 264, respectively. The normalized adsorption equilibrium time obtained from an Intelligent Gravimetric Analyzer (IGA) was used to compare the adsorption kinetics rates among samples with different morphologies. The relevant dynamic breakthrough experiments indicate that this hierarchical pore structure facilitates the separation performance with an excellent CO2 adsorption capacity. This study provides a new strategy for the design of high-efficiency adsorbents. Although some aspects of adsorption kinetics in CHA zeolites have been studied, there is still a lack of research that systematically describes the CO2 adsorption behavior of CHA using kinetic equations. Therefore, this paper uses H-type FAU zeolite molecular sieves as raw materials to explore the synthesis conditions for CHA molecular sieves by crystallization and to study the carbon dioxide adsorption kinetics and thermodynamics of the prepared CHA molecular sieves.
1　Experimental
Less
1.1　Preparation of CHA zeolite
The HY zeolite (SiO2/Al2O3 molar ratio=5) was purchased from the Nankai University Catalyst Co., Ltd. Potassium hydroxide (KOH, 98%, Purchased from Greagent). The deionized water was prepared in the laboratory.
The specific synthesis process is as follows: first, deionized water, potassium hydroxide and HY (SiO2/Al2O3=5) zeolite sieve are added to the polytetrafluoroethylene lining of the hydrothermal synthesis reactor, and then the mixture is continuously magnetically stirred for 1 h at room temperature. Then, the polytetrafluoroethylene liner containing the mixture was placed in a stainless steel high-pressure reactor. The high-pressure reactor was sealed and moved into a preheated oven. After hydrothermal synthesis at 423 K for 48 h, it was taken out and rapidly cooled. The obtained solid sample was taken out, washed with deionized water until neutral, and dried at 373K for 8 h to obtain CHA zeolite.
1.2　Characterization of CHA zeolite
The crystal structure of the synthesized sample was characterized using XRD (Panalytial X’Pert Powder, Netherlands). The XRD pattern was recorded on a Panalytial X’ Pert Powder diffractometer using a Cu Kα radiation source (λ=1.5406 Å) to characterize the powder. The step size was 0.013° and the scan was performed once every 0.109(°)/s in the 2θ range of 5°−50°. Gas adsorption tests were conducted at 273 and 298 K using a BSD-660M physical adsorption instrument manufactured by Best Instruments Co., Ltd. The surface morphology and aggregation state of the synthesized samples were observed using a thermal field emission scanning electron microscope (ZEISS Gemini SEM 300). The accelerating voltage was 200 V−30 kV, the resolution was 1.2 nm, and the magnification was 25−200000 to obtain the scanning electron microscope (SEM) images. Elemental quantitative analysis of the HY molecular sieve raw material for crystal transformation was performed using XRF (XRF-1800). The relative crystallinity of the molecular sieve was calculated using Highscore Plus software based on the intensity of the main characteristic peaks (2θ=9.45°, 12.83°, 15.93°, 20.49°, 30.49°) in the XRD pattern. The specific calculation formula is as follows:
$ \mathrm{Relative}~\text{crystallinity}\left(\mathrm{\% }\right)=\frac{\mathrm{The}~\mathrm{sum}~\mathrm{of}~\mathrm{the}~\mathrm{characteristic}~\mathrm{peak}~\mathrm{areas}~\mathrm{of}~\mathrm{the}~\text{samples}}{\mathrm{The}~\mathrm{sum}~\mathrm{of}~\mathrm{the}~\mathrm{characteristic}~\mathrm{peak}~\mathrm{areas}~\mathrm{of}~\mathrm{the}~\mathrm{standard}~\text{samples}}\times 100\% $
1.3　Gas adsorption performance test
The static adsorption performance was tested using a BSD-660M physical adsorption instrument from BeiShiDe Instruments. First, the test sample was activated at 523 K under vacuum for 6 h, and then its nitrogen and carbon dioxide gas adsorption isotherms were measured at 273 and 298 K, respectively. To examine the CO2/N2 separation capability of cha zeolite, the CO2/N2 (20∶80) adsorption selectivity was calculated based on single-component gas adsorption isotherm data. First, the pure component isotherm data of CO2 and N2 recorded at 273 and 298 K were fitted using the Dual-Site Langmuir-Freundlich (DSLF) model:
$ q={q}_{{\mathrm{A,sat}}}\frac{{b}_{{{{\mathrm{A}}}}}{p}^{{{v}_{{{{\mathrm{A}}}}}}}}{1+{b}_{{{{\mathrm{A}}}}}{p}^{{{v}_{{{{\mathrm{A}}}}}}}}+{q}_{{\mathrm{B,sat}}}\frac{{b}_{{{{\mathrm{B}}}}}{p}^{{{v}_{{{{\mathrm{B}}}}}}}}{1+{b}_{{{{\mathrm{B}}}}}{p}^{{{v}_{{{{\mathrm{B}}}}}}}} $
where q is the component molar loading (mol/kg), qA,sat and qB,sat are the saturated component molar loadings at adsorption sites A and B (mol/kg), respectively. p is the total system pressure at equilibrium (kPa), while bA and bB are Langmuir-Freundlich constant at sites A and B (1 kPa−1). The parameters νA and νB represent the reciprocal of deviations from an ideal homogeneous surface[15].
The gas selectivity was calculated based on the Ideal Solution Theory (IAST). Based on the isotherms of the pure components, the adsorption capacity of CHA zeolite for both gases in the CO2/N2 (20∶80) mixture was determined by applying the fitting equation (Figure S1), and the selectivity was calculated using the following formula:
$ {\mathrm{Selectivity}}=\frac{{q}_{{\mathrm{C}}{{{\mathrm{O}}}_{2}}}/{q}_{{{{\mathrm{N}}}_{2}}}}{{y}_{{\mathrm{C}}{{{\mathrm{O}}}_{2}}}/{y}_{{{{\mathrm{N}}}_{2}}}}\times 100\% $
where $q_{{\mathrm{CO}}_2} $ and $q_{{\mathrm{N}}_2} $ are the uptakes, and $y_{{\mathrm{CO}}_2} $ and $y_{{\mathrm{N}}_2} $ are the partial pressure of components 1 and 2, respectively[16].
The dynamic adsorption performance was tested on a specific gas adsorption and separation experimental apparatus (SIRIUS-HG-40G). First, the molecular sieve is compressed into tablets to screen out particles of 40−60 mesh. Then, it is loaded into an adsorption tube and activated at 523 K under vacuum for 6 h before being cooled to room temperature. Pure CO2 or a mixture of 20% CO2 and 80% N2 was introduced into the gas adsorption separation apparatus at room temperature using a mass flow meter at a specific flow rate. The gas concentration at the end of the penetration column was measured using an online mass spectrometer. The temperature during the experiment was controlled by a circulating water bath. The dynamic gas adsorption capacity and gas selectivity were calculated according to the following equations (4) and (3), respectively.
$ q=\frac{F\times {C}_{0}\times \displaystyle\int \limits_{0}^{{t}_{i}}\left(1-\dfrac{{C}_{t}}{{C}_{0}}\right){\mathrm{d}}t}{m} $
where q is the saturated adsorption capacity of a certain component gas; m is the adsorbent mass; C0 is the gas inlet concentration; Ct is the gas outlet concentration at time t; ti is the adsorption time; and F is the total gas flow rate.
1.4　CO2 adsorption kinetics analysis
The adsorption column breakthrough experiment[17−18] was conducted on a specific gas adsorption separation experimental apparatus (SIRIUS-HG-40G). CO2 kinetic curves were measured at 298, 323 and 348 K, and the curves were fitted using pseudo-first-order kinetic equations, pseudo-second-order kinetic equations, and the Avrami kinetic model respectively[19−20].
Pseudo-first-order adsorption kinetics model, which describes the adsorption process in terms of adsorption capacities, is among the most widely employed rate models in adsorption studies. It is described as follows[21]：
$ {q}_{t}=a(1-{{\mathrm{e}}}^{-{{k}_{1}}t}) $
where qt is the adsorption at time t, a is the adsorption at adsorption equilibrium, k1 is the pseudo-first-order adsorption kinetic parameter and t is time.
Pseudo-second-order adsorption kinetic model is based on the assumption that the adsorption capacity is proportional to the number of occupied active sites on the adsorbent surface[22]. The model is commonly expressed as：
$ {q}_{t}=\frac{{a}^{2}{k}_{1}t}{1+a{k}_{2}t} $
where, qt is the adsorption at time t, a is the adsorption at adsorption equilibrium, k1 and k2 are pseudo-second-order adsorption kinetic parameters, and t is time.
Avrami adsorption kinetic model was initially developed to describe particle nucleation. Recently, this model has been extended to simulate phase transitions and crystal growth in materials, as well as to investigate the dynamic adsorption behavior of solid adsorbents[18,23−24]. The model is expressed as：
$ {q}_{t}=a(1-{{\mathrm{e}}}^{-(kt{{)}^{n}}}) $
where qt is the amount of adsorbent adsorbed at time t, a is the equilibrium adsorption amount, k is the adsorption rate constant, t is time，and n is the Avrami exponent, which is often in fractional form, and reflects possible mechanism changes in the adsorption process[25]. The parameter n characterizes the dimensional growth of adsorbed species at the active site, with n = 2 corresponding to one-dimensional growth, n = 3 indicating two-dimensional growth, and higher values representing progressively higher-dimensional expansion[26]. For uniform adsorption, where the probability of adsorption is equal across all zones within a fixed time interval, n = 1[27]. When n = 2, the adsorption process represents an ideal one-dimensional growth initiated from the adsorption site on the adsorbent surface, characterized by continuous formation and a constant rate[26]. The fractional order of this model arises due to the complexity of the reaction mechanism or the simultaneous occurrence of multiple reaction pathways[28].
Calculation of adsorption activation energy using the Arrhenius equation[29]:
$ k={k}_{0}{{\mathrm{e}}}^{\left(\tfrac{E}{RT}\right)} $
where k0 is the adsorption rate constant, E is the adsorption activation energy, R is the gas constant, and T is the absolute temperature.
1.5　Thermodynamic analysis of CO2 adsorption
The adsorption heat of CO2 is calculated using the Virial equation[30], and its expression is shown in (9).
$ \ln p=\ln N+\frac{1}{T}{\sum \limits}_{i=0}^{m}{a}_{i}{N}^{i}+{\sum \limits}_{j=0}^{n}{b}_{j}{N}^{j} $
In the formula, p is the pressure (unit: bar), N is the adsorption amount (unit: mmol/g), T is the temperature (unit: K); ai and bj are temperature-independent Virial coefficients, and m and n are the number of terms required to describe the isotherm.
Based on the above equation, the adsorption heat Qst is calculated using the Virial coefficients a0 to am:
$ {Q}_{{\mathrm{st}}}=-R{\sum \limits}_{i=0}^{m}{a}_{i}{N}^{i} $
where Qst is the heat of adsorption and R is the gas constant.
2　Results and discussion
Less
2.1　CHA synthesis conditions
2.1.1　Study of n(KOH)/n(SiO2) on synthesis
As shown in Figure 1, the XRD and SEM were applied to investigate the effect of the basicity ratio n(KOH)/n(SiO2) on zeolite structure in the synthesis system. When n(KOH)/n(SiO2) = 0.5, weak CHA zeolite characteristic diffraction peaks can be observed in the XRD pattern, while the SEM image shows that the bulk HY zeolite has agglomerated. This indicates that a higher basicity ratio is required to completely dissolve HY zeolite and convert it into CHA molecular sieve.
When n(KOH)/n(SiO2) increases to 0.6, pure-phase CHA zeolite is obtained, and the blocky particles constituting the spiky structure are evenly distributed in the SEM image. However, when the alkalinity ratio was further increased to 0.7 and 0.8, the relative crystallinity of the samples decreased significantly (Table 1), and the blocky particles in the spiky structure tended to be finer, with the diameter of the spheres decreasing (Figure 1). The reduced crystallinity and altered morphology may result from the partial dissolution of CHA molecular sieve caused by excessive alkalinity.
2.1.2　Study of n(H2O)/n(SiO2) on synthesis
Based on the results in the previous step, the influence of n(H2O)/n(SiO2) ratios on the structure and morphology of CHA zeolite was studied under the condition of n(KOH)/n(SiO2) = 0.6. The XRD pattern in Figure 2 shows that as the ratio increases to 110, a distinct characteristic peak of HY zeolite appears at 2θ=6.2°. When the ratio is further increased to 130, the intensity of this characteristic peak is significantly enhanced. This is attributed to the reduced activity of OH− under high water content, preventing the complete dissolution of HY crystals. At the same time, the probability of the effective collision between K+ and soluble (aluminum) silicate oligomers (such as four-membered ring structural units) is reduced, hindering the formation of the CHA cage structure. SEM (Figure 2(b)−(f)) show that as the water content of the system increases, the surface morphology of as-synthesized zeolites exhibits a gradual evolution: under low water content, excessive alkali solution will corrode the CHA crystal nuclei, causing the resultant spheres appear spread out with sparsely protrusion. At a n(H2O)/n(SiO2) of 110, although the crystal retains a spherical outline, it still contains a large number of blocky fragments and fine HY zeolite particles. When the ratio is further increased to 130, the microspheres are mainly composed of regular hexagonal or smooth sheet-like HY single crystals. It is worth noting that the diameter of the sphere decreases monotonically with increasing water content. The optimal relative crystallinity value was obtained at a H2O/SiO2 ratio of 90 (Table 1), confirming that this condition is most favorable for the synthesis of CHA molecular sieves.
2.1.3　Study of crystallization temperature on synthesis
Considering the effect of crystallization conditions (Figure 3) and the corresponding performance parameters, it is evident that crystallization temperature plays an insignificant role under optimal time and alkalinity conditions. Within the crystallization temperature range of 393 to 433 K, all characteristic peaks of CHA molecular sieves can be clearly detected in the XRD patterns (Figure 3(a)), indicating that the formation of a pure CHA phase across this temperature range. When the crystallization temperature gradually increases, the relative crystallinity of the product shows a volcanic trend, reaching a peak (Table 1) at 423 K. The relevant SEM images (Figure 3 (b)−(f)) further revealed the regulatory effect of crystallization temperature on zeolite morphology: at lower crystallization temperatures, the samples exist in the form of scattered small fragments with poor dispersion, and the surface crystal exhibits a primary disk shape. The measured crystal grain size is about 0.8 μm. As indicated by XRD analysis, the scattered fragments are pure CHA. As the synthesis temperature increases, the crystal morphology gradually transforms from disk-shaped and rhomboid to cluster-shaped. The size of the bulk CHA crystals gradually increases and they assemble into spherical aggregates through agglomeration, while the crystallinity of the product increases simultaneously. Among them, the crystals prepared at 423 K exhibited a more symmetrical and regular spherical morphology.
2.1.4　Study of crystallization time on CHA synthesis
As shown in Figure 4 and Table 1, the crystallization process is incomplete after 24 h, as indicated by the presence of FAU phase (from HY zeolite) present in the XRD pattern. When the crystallization time reached 36 h, the intensity of the characteristic peak of HY zeolite decreased significantly, while the characteristic peak of CHA-type molecular sieve began to appear. This phase transformation can be explained by the structure-directing effect of K+ during prolonged crystallization. The system reaches crystallization equilibrium at 48 h, with the crystallinity reaching its maximum. At this point, the crystal growth rate and dissolution rate are in dynamic equilibrium. It is worth noting that extending the crystallization time to 72 h resulted in a slight decrease in crystallinity, which is related to the metastable nature of molecular sieves[31].
Based on the evolution pattern analysis in Figure 4, the crystallization CHA molecular sieve can be divided into four stages: (1) Initial stage (0–24 h): In the early stage of crystallization, HY zeolite dissolves under alkaline conditions[32−33]. The dissolution rate is affected by various factors such as temperature, basicity, silica-alumina ratio, and reactant concentration. K+ ions may act as structure-directing agents or crystallization aids at this stage, promoting the aggregation and agglomeration of dissolved components (such as silicate and aluminate species) to form amorphous or nanocrystalline intermediates[32]. (2) Reorganization stage (24–36 h): HY zeolite continues to dissolve, while the internal structure of the spherical aggregates is reconstructed with a pronounced increase in crystallinity. In this stage, the aggregates (or gel particles) formed by the initial dissolved components begin to undergo internal structural rearrangement and crystallization. Meanwhile, the remaining HY zeolite in the solution continues to dissolve, providing more silicon and aluminum sources for the newly formed CHA crystals[34]. The sharp increase in crystallinity indicates an accelerated formation rate of the CHA phase, with the nuclei of the new phase growing rapidly inside or on the surface of the aggregates. This typically involves the synergistic effect of solution phase transformation and solid-phase rearrangement[35]. Some studies have also mentioned that under hydrothermal conditions, materials undergo a transformation from amorphous to crystalline phase over time, accompanied by structural reorganization[36]. (3) Crystal growth period (36–48 h): During this period, the dissolution of HY zeolite stops, and the system enters the pure crystal growth stage, with the grain size on the surface of the spheres increasing linearly. After most of the precursors dissolve and are converted into CHA crystal nuclei, the system enters the crystal growth-dominated stage[34]. At this point, the silicon and aluminum species in the supersaturated solution continue to deposit onto the surface of the formed crystal nuclei, resulting in an increase in grain size[37]. The crystal growth rate may remain relatively stable, resulting in a linear increase in grain size. (4) Late crystallization stage (48–72 h): In the late crystallization stage (48–72 h), since crystal growth has reached its limit, the system undergoes reverse dissolution, which manifests as a reduction in the diameter of the spheres and a decrease in the size of the surface grains[38].
Based on the analysis presented above, the optimal synthesis conditions for CHA were subsequently determined: n(KOH)/n(SiO2) = 0.6, n(H2O)/n(SiO2) = 90, crystallization temperature of 423 K, synthesis time of 48 h. This combination of parameters achieves an optimal balance between crystal phase purity, crystallinity, and energy efficiency, laying the foundation for subsequent testing and analysis. Since crystal size and Si/Al ratio significantly impact the adsorption performance of materials, samples with distinct morphologies were selected for preliminary adsorption performance tests (Figure S2) and elemental composition analysis (Table S1). Considering the above factors comprehensively, the CHA sample prepared under the conditions of n(KOH)/n(SiO2) = 0.6, n(H2O)/n(SiO2) = 90, a crystallization temperature of 423 K, and a synthesis time of 48 h was selected for further detailed analysis of its adsorption performance.
2.2　CO2 adsorption performance and mechanism analysis of CHA zeolite
The dynamic and static adsorption properties of the prepared CHA zeolite were tested. As shown in the Figure 5(a), dynamic adsorption tests indicate that within the temperature range of 273−323 K, the adsorption capacity of CHA zeolite decreases with increasing temperature. The gas adsorption capacity decreased from 4.04 mmol/g at 273 K to 3.3 mmol/g at 423 K. The same trend was observed in the static adsorption data as shown in Figure 5(b). The adsorption capacities of CO2 and N2 at 298 K were lower than those at 273 K. This reduction may be due to the fact that adsorption is an exothermic process, and the adsorbed CO2 is desorbed as the temperature increases[39].
The breakthrough experiments were conducted using a CO2/N2 mixture (20∶80, V/V) to analyze the adsorption capacity and separation coefficient of CO2 and N2 (Figure 5(c)). The breakthrough data revealed distinct adsorption behaviors at key points. At the breakthrough point (5%), the corresponding CO2 and N2 uptake were 3.22 and 0.21 mmol/g respectively, with a separation coefficient of 59.96. As the breakthrough process proceeds, the material's selectivity for CO2 successively decreases at the semi-dry point (50%), flow-dry point (95%), and the equilibrium point, ultimately reaching 26.91% of its value at the equilibrium point. The separation coefficient decreases as penetration progresses. The analysis of the breakthrough curve of the mixed gas should also include an overall analysis of the breakthrough process. The material displayed a prominent selective adsorption for CO2 with a breakthrough time of 2464.6 s/g, while N2 reached the flow point much earlier at 106.2 s/g. Comprehensive analysis showed that when the penetration reached 2464.6 s/g, the N2 gas curve showed a C/C0 greater than 1. This is because the interaction force between CO2 and the material is stronger than that between CO2 and N2.
As adsorption proceeds, CO2 gas molecules will displace the previously adsorbed N2 molecules and occupy the adsorption sites. Consequently, the separation coefficient under actual mixed-gas equilibrium conditions is greater than 26.91, the value calculated from individually measured equilibrium uptakes.
For the static data analysis, the adsorption isotherms at different temperatures were fitted using the DSLF equation (Figure S3), the adsorption uptake (Figure S1) and the CO2/N2 selectivity under mixed-gas condition (CO2/N2=20∶80) was calculated using the ideal solution theory (IAST). IAST data show (Figure 5(d)) that at different temperatures (273 and 298 K), the selectivity exhibits a trend of increasing selectivity with increasing adsorption pressure. Furthermore, the selectivity at 298 K is much higher than that at 273 K. This may be because higher temperature promotes gas molecular activity, allowing CO2 to preferentially occupy more adsorption sites. This indicates that the material's selectivity for gases is primarily driven by kinetic effects[40].
2.3　Adsorption kinetics analysis of CO2 in CHA zeolite
A detailed kinetic analysis was performed on the prepared CHA zeolite. The adsorption data at 298 K were fitted and analyzed using pseudo-first-order kinetic equations, pseudo-second-order kinetic equations, and the Avrami equation (Figure 6(a)). When pseudo-first-order and pseudo-second-order kinetic equations are used, the obtained R2 is significantly lower (Table 2), indicating that these two models cannot effectively describe the adsorption kinetic characteristics. In contrast, the Avrami equation showed the best fit to the adsorption data with an R2 of 0.9946, demonstrating its greater suitability for analyzing the kinetic behavior of this system (Figure 6(b)). Upon the Avrami equation, the adsorption rate constant increases continuously with increasing temperature (Figure 6(c),Table 3), indicating that the adsorption rate is enhanced with increasing temperature. This suggests that the adsorption process can reach equilibrium more quickly at higher temperatures. The corresponding adsorption activation energy of CHA zeolite for CO2 was calculated to be 8.31 kJ/mol (Figure 6(d)). This value indicates that the adsorption process is dominated by physisorption.
2.4　Thermodynamic analysis of CO2 adsorption in CHA zeolite
In thermodynamic studies of adsorption processes, the heat of adsorption indicating the strength of the interaction between the adsorbate and the adsorbent, is a key parameter for evaluating the energy characteristics of the adsorption process and understanding the adsorption mechanism and designing adsorption cycles.
In this study, the adsorption heat of CO2 was calculated by fitting the experimental data to the virial equation using AIM software[41], enabling an in-depth exploration of the adsorption mechanism.
The virial equation was specifically proposed to describe the relationship between adsorption amount and operational parameters (pressure and temperature), and can be directly used to calculate the heat of adsorption of equal amounts and its behavior under different conditions[42]. The CO2 adsorption isotherms at 273 and 298 K were fitted using the virial equation to obtain relevant fitting parameters (Figure 7). Then, the CO2 adsorption heat data of CHA molecular sieve were calculated based on the obtained parameters. Adsorption heat data show that the adsorption heat varies with different adsorption amounts, indicating that the CHA molecular sieve has a heterogeneous surface. However, the overall adsorption heat is below 20 kJ/mol（Figure 7）, which is considered physical adsorption. Kinetic data also confirm this, showing that the interaction force between CO2 and CHA is relatively small, which helps reduce the energy consumption of the desorption process.
3　Conclusion
Less
This study successfully synthesized CHA zeolite under optimized conditions (n(KOH)/n(SiO2) = 0.6, n(H2O)/n(SiO2) = 90, hydrothermal synthesis temperature 423 K, hydrothermal synthesis time 48 h) using the H-FAU zeolite crystallization method. The CO2 adsorption performance of CHA zeolite was tested in detail. Dynamic adsorption test data show that under the conditions of 1 bar and 273−323 K, the CO2 adsorption capacity decreases with increasing temperature, from 4.04 mmol/g at 273 K to 3.3 mmol/g at 323 K. Static adsorption data show that at 1 bar, the CO2 adsorption capacity also exhibits a decreasing trend with increasing temperature at 273 and 298 K, indicating that the adsorption process is exothermic. Thermodynamic analysis using the virial equation to calculate the heat of adsorption during the adsorption process, further confirmed that the adsorption process is exothermic. In the IAST selectivity calculation, the selectivity of CHA zeolite for CO2 increases with increasing temperature, indicating that the separation process is mainly affected by diffusion. Furthermore, the breakthrough curve shows C/C0 bigger than 1 at the end of the breakthrough column, suggesting that the interaction strength between CHA zeolite and CO2 is greater than that with N2. These findings provide insights into improving the separation efficiency of CHA zeolite in practical separation processes, demonstrating its significant application potential.
References
Less
1
SCHIMEL D S. The carbon equation[J]. Nature, 1998, 393(6682): 208−209.
2
KARIMI M, SHIRZAD M, SILVA J A, et al. Carbon dioxide separation and capture by adsorption: A review[J]. Environ Chem Lett, 2023, 21(4): 2041−2084.
3
ABD A A, NAJI S Z, HASHIM A S, et al. Carbon dioxide removal through physical adsorption using carbonaceous and non-carbonaceous adsorbents: A review[J]. Environ Chem Eng, 2020, 8(5): 104142.
4
FU D, DAVIS M E. Carbon dioxide capture with zeotype materials[J]. Chem Soc Rev, 2022, 51(22): 9340−9370.
5
INDIRA V, ABHITHA K. A review on recent developments in zeolite a synthesis for improved carbon dioxide capture: Implications for the water-energy nexus[J]. Energy Nexus, 2022, 7: 100095.
6
PAN H, YU C, SUO X, et al. Emerging porous materials for carbon dioxide adsorptive capture: Progress and challenges[J]. Mater Chem Front, 2023, 7(24): 6463−6482.
7
CLATWORTHY E B, GHOJAVAND S, GUILLET-NICOLAS R, et al. Dynamic adsorption of CO2 by CHA zeolites-size matters[J]. Chem Eng J, 2023, 471: 144557.
8
YANG J, LIU J, LIU P, et al. K‐Chabazite zeolite nanocrystal aggregates for highly efficient methane separation[J]. Angew Chem Int Ed, 2022, 61(8): e202116850.
9
YUE B, LIAN X, LIU S, et al. Efficient nitrous oxide capture by cationic forms of FAU and CHA zeolites[J]. Chem Eng J, 2023, 462: 142300.
10
SHANG J, LI G, SINGH R, et al. Discriminative separation of gases by a “molecular trapdoor” mechanism in chabazite zeolites[J]. J Am Chem Soc, 2012, 134(46): 19246−19253.
11
WANG X, ZHENG D, GUO J, et al. Inverse CO2‐C2H2 separation on the low‐silica CHA zeolite through cooperative cation and gas molecule migration mechanism[J]. Angew Chem Int Ed, 2025: e22386.
12
LIU S, LIAN X, YUE B, et al. Control of zeolite local polarity toward efficient xenon/krypton separation[J]. J Am Chem Soc, 2024, 146(12): 8335−8342.
13
FU D, PARK Y, DAVIS M E. Zinc containing small‐pore zeolites for capture of low concentration carbon dioxide[J]. Angew Chem Int Ed, 2022, 61(5): e202112916.
14
CAO S, LI L, GUO M, et al. Construction of sunflower-like superstructure of cha zeolite through oriented attachment for superior CO2 separation performance via thermodynamic–kinetic synergistic adsorption[J]. Chem Mater, 2023, 35(23): 10119−10128.
15
GAO J, CAI Y, QIAN X, et al. A microporous hydrogen‐bonded organic framework for the efficient capture and purification of propylene[J]. Angew Chem Int Ed, 2021, 133(37): 20563−20569.
16
ZHANG X, LI L, WANG J-X, et al. Selective ethane/ethylene separation in a robust microporous hydrogen-bonded organic framework[J]. J Am Chem Soc, 2019, 142(1): 633−640.
17
SERNA-GUERRERO R, SAYARI A. Modeling adsorption of CO2 on amine-functionalized mesoporous silica. 2: Kinetics and breakthrough curves[J]. Chem Eng J, 2010, 161(1/2): 182−190.
18
LIU Y, YU X. Carbon dioxide adsorption properties and adsorption/desorption kinetics of amine-functionalized KIT-6[J]. Appl Energy, 2018, 211: 1080−1088.
19
CHEN X. Study on high-temperature CO2 adsorption characteristics and reaction kinetics of doped lithium silicate adsorbent[D]. Huazhong University of Science and Technology, 2018.
20
CHEN S. CO2 Adsorption performance and kinetics of novel amino-modified solid adsorbents[D]. Changsha: Hunan University, 2021.
21
SIRCAR S, HUFTON J. Why does the linear driving force model for adsorption kinetics work?[J]. Adsorption, 2000, 6(2): 137−147.
22
HO Y-S, MCKAY G. Pseudo-second order model for sorption processes[J]. Process Biochem, 1999, 34(5): 451−465.
23
LIU Q, SHI J, WANG Q, et al. Carbon dioxide capture with polyethylenimine-functionalized industrial-grade multiwalled carbon nanotubes[J]. Ind Eng Chem Res, 2014, 53(44): 17468−17475.
24
CHEN S P, SUN X, LUO X, et al. CO2 adsorption on premodified Li/Al hydrotalcite impregnated with polyethylenimine[J]. Ind Eng Chem Res, 2018, 58(3): 1177−1189.
25
DE MENEZES E W, LIMA E C, ROYER B, et al. Ionic silica based hybrid material containing the pyridinium group used as an adsorbent for textile dye[J]. Colloid Interface Sci, 2012, 378(1): 10−20.
26
BENEDICT J B, COPPENS P. Kinetics of the single-crystal to single-crystal two-photon photodimerization of α-trans-cinnamic acid to α-truxillic acid[J]. Phys Chem A, 2009, 113(13): 3116−3120.
27
AVARAMI M. Granulation, phase change and microstructure III: Kinetics of phase change[J]. J Chem Phys, 1941, 9: 177−184.
28
CESTARI A R, VIEIRA E F, VIEIRA G S, et al. The removal of anionic dyes from aqueous solutions in the presence of anionic surfactant using aminopropylsilica—A kinetic study[J]. Hazard Mater, 2006, 138(1): 133−141.
29
ZHAO G. Synthesis and adsorption and catalytic properties of hydrophobic mesoporous materials containing perfluorocarbon chains[D]. Guangzhou: South China University of Technology, 2014.
30
BAI R, YAN N, HE G, et al. Ethylene pretreatment enhances ethylene adsorption and separation over Cu@ SAPO‐RHO zeolite[J]. Angew Chem Int Ed, 2025, 64(22): e202501053.
31
LI Y, HU N, ZHANG F, et al. Rapid synthesis of low-silica ribbonite molecular sieves induced by heterogeneous seeds[J]. Inorg Chem, 2018, 34(12): 2143−2152.
32
GOTO I, ITAKURA M, SHIBATA S, et al. Transformation of LEV-type zeolite into less dense CHA-type zeolite[J]. Microporous Mesoporous Mater, 2012, 158: 117−122.
33
HIGUCHI Y, TANAKA S. Interzeolite transformation from H+-type FAU zeolite into pure CHA zeolite via OSDA/seeds-free and steam-assisted conversion process[J]. Microporous Mesoporous Mater, 2023, 354: 112550.
34
ASGAR POUR Z, ALASSMY Y A, SEBAKHY K O. A survey on zeolite synthesis and the crystallization process: Mechanism of nucleation and growth steps[J]. Crystals, 2023, 13(6): 959.
35
DO M H, WANG T, CHENG D-G, et al. Zeolite growth by synergy between solution-mediated and solid-phase transformations[J]. Mater Chem A, 2014, 2(35): 14360−14370.
36
BELLO-JURADO E, MILLET I, VAN TENDELOO L, et al. Enhancing nucleation to synthesize Al-rich CHA zeolites under ultra-low OSDA contents: Application for heavy-duty NH3-SCR of NOx[J]. Microporous Mesoporous Mater, 2024, 371: 113071.
37
ZHANG S, HU J, WANG Y, et al. Organic template-free synthesis of CHA zeolite by hydrothermal conversion of magadiite with the assistance of seeds and an investigation of crystallization mechanism[J]. Microporous Mesoporous Mater, 2024, 380: 113297.
38
TSUNOJI N, ONISHI M, SONODA S, et al. Synthesis‐structure‐catalysis relations in CHA zeolites applied for selective catalytic reduction of NOx with ammonia[J]. ChemCatChem, 2024, 16(16): e202400459.
39
WELDEKIDAN H, PATEL H, MOHANTY A, et al. Synthesis of porous and activated carbon from lemon peel waste for CO2 adsorption[J]. Carbon Capture Sci Technol, 2024, 10: 100149.
40
BA Y-Q, WANG Y-S, LI T-Y, et al. Fine tuning CO2 adsorption and diffusion behaviors in ultra-microporous carbons for favorable CO2 capture at moderate temperature[J]. Sust Chem Clim Action, 2023, 2: 100015.
41
HASSAN M, YOON S, CHEN Y, et al. AIM: A user-friendly GUI workflow program for isotherm fitting, mixture prediction, isosteric heat of adsorption estimation, and breakthrough simulation[J]. Phys Statistical Mechanics, 2025, 29: 4.
42
CZEPIRSKI L, JAGIEŁŁO J. Virial-type thermal equation of gas—solid adsorption[J]. Chem Eng Sci, 1989, 44(4): 797−801.
Appendix
Less
Year 2026 volume 54 Issue 9
PDF
219
108
Cite this Article
BibTeX
Article Info
doi: 10.1016/S1872-5813(26)60687-1
  • Receive Date：2025-12-09
  • Online Date：2026-09-23
  • Published：2026-09-10
Article Data
Affiliations
History
  • Received：2025-12-09
  • Revised：2026-01-11
  • Accepted：2026-01-27
Affiliations
    1State Key Laboratory of Heavy Oil Processing, CNPC Key Laboratory of Catalysis, School of Chemical Engineering and Environmental Science, China University of Petroleum (Beijing), Beijing 102249, China
    2CNPC Key Laboratory of Catalysis, Petrochemical Research Institute, Lanzhou 730060, China

Corresponding:

Tel: 010-89732316, E-mail:
References
Share
https://castjournals.cast.org.cn/joweb/rlhxxb/EN/10.1016/S1872-5813(26)60687-1
Share to
QR

Scan QR to access full text

Cite this article
BibTeX
Citations
表12种不同金属材料的力学参数
科
Family		 属数
Number of
genus		 种数
Number of
species		 占总种数比例
Percentage of
total species (%)		 属
Genus		 种数
Number of
species		 占总种数比例
Percentage of total
species (%)
鹅膏菌科Amanitaceae 2 11 5.26 鹅膏菌属 Amanita 10 4.78
小菇科 Mycenaceae 2 12 5.74 丝盖伞属 Inocybe 5 2.39
多孔菌科 Polyporaceae 8 14 6.70 蜡蘑属 Laccaria 5 2.39
红菇科 Russulaceae 3 23 11.00 小皮伞属 Marasmius 6 2.87
小菇属 Mycena 11 5.26
光柄菇属 Pluteus 5 2.39
红菇属 Russula 17 8.13
栓菌属 Trametes 5 2.39
关闭全屏
  • BibTeX
  • EndNote
  • RefWorks
  • TxT
Links
Articles
Latest Articles
Most Read
Collections
Updates
Events
News
Multimedia
About
About Us
Contact
No. 86 Xueyuan South Road, Haidian District, Beijing
100081
010-62662699(Operation and Technical Support)
qkjq@cast.org.cn

Copyright © 2025 China Association for Science and Technology. All rights reserved. For all open access content, the relevant licensing terms apply.
Sponsored by the Office of the Leading Group for Cybersecurity and Informatization of CAST, and supported by Science and Technology Review Publishing House